The rate of reaction increases isgnificantly with increase in temperature. Generally, rate of reactions are doubled for every `10^(@)C` rise in temperature. Temperature coefficient gives us an idea about the change in the rate of a reaction for every `10^(@)C` change in temperature. `"Temperature coefficient" (mu) = ("Rate constant of" (T + 10)^(@)C)/("Rate constant at" T^(@)C)` Arrhenius gave an equation which describes aret constant `k` as a function of temperature `k = Ae^(-E_(a)//RT)` where `k` is the rate constant, `A` is the frequency factor or pre-exponential factor, `E_(a)` is the activation energy, `T` is the temperature in kelvin, `R` is the universal gas constant. Equation when expressed in logarithmic form becomes `log k = log A - (E_(a))/(2.303 RT)` For the given reactions, following data is given `{:(PrarrQ,,,,k_(1) =10^(15)exp((-2000)/(T))),(CrarrD,,,,k_(2) = 10^(14)exp((-1000)/(T))):}` Temperature at which `k_(1) = k_(2)` isA. `434.22 K`B. `1000 K`C. `2000 K`D. `868.44 K`